Classifications

• • B—PERFORMING OPERATIONS; TRANSPORTING
  • B22—CASTING; POWDER METALLURGY
  • B22F—WORKING METALLIC POWDER; MANUFACTURE OF ARTICLES FROM METALLIC POWDER; MAKING METALLIC POWDER; APPARATUS OR DEVICES SPECIALLY ADAPTED FOR METALLIC POWDER
  • B22F9/00—Making metallic powder or suspensions thereof
  • B22F9/16—Making metallic powder or suspensions thereof using chemical processes
  • B22F9/18—Making metallic powder or suspensions thereof using chemical processes with reduction of metal compounds
  • B22F9/20—Making metallic powder or suspensions thereof using chemical processes with reduction of metal compounds starting from solid metal compounds
  • B22F9/22—Making metallic powder or suspensions thereof using chemical processes with reduction of metal compounds starting from solid metal compounds using gaseous reductors
• • B—PERFORMING OPERATIONS; TRANSPORTING
  • B22—CASTING; POWDER METALLURGY
  • B22F—WORKING METALLIC POWDER; MANUFACTURE OF ARTICLES FROM METALLIC POWDER; MAKING METALLIC POWDER; APPARATUS OR DEVICES SPECIALLY ADAPTED FOR METALLIC POWDER
  • B22F9/00—Making metallic powder or suspensions thereof
  • B22F9/16—Making metallic powder or suspensions thereof using chemical processes
  • B22F9/30—Making metallic powder or suspensions thereof using chemical processes with decomposition of metal compounds, e.g. by pyrolysis
• • B—PERFORMING OPERATIONS; TRANSPORTING
  • B82—NANOTECHNOLOGY
  • B82Y—SPECIFIC USES OR APPLICATIONS OF NANOSTRUCTURES; MEASUREMENT OR ANALYSIS OF NANOSTRUCTURES; MANUFACTURE OR TREATMENT OF NANOSTRUCTURES
  • B82Y30/00—Nanotechnology for materials or surface science, e.g. nanocomposites
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01B—NON-METALLIC ELEMENTS; COMPOUNDS THEREOF; METALLOIDS OR COMPOUNDS THEREOF NOT COVERED BY SUBCLASS C01C
  • C01B13/00—Oxygen; Ozone; Oxides or hydroxides in general
  • C01B13/14—Methods for preparing oxides or hydroxides in general
  • C01B13/18—Methods for preparing oxides or hydroxides in general by thermal decomposition of compounds, e.g. of salts or hydroxides
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01F—COMPOUNDS OF THE METALS BERYLLIUM, MAGNESIUM, ALUMINIUM, CALCIUM, STRONTIUM, BARIUM, RADIUM, THORIUM, OR OF THE RARE-EARTH METALS
  • C01F7/00—Compounds of aluminium
  • C01F7/02—Aluminium oxide; Aluminium hydroxide; Aluminates
  • C01F7/30—Preparation of aluminium oxide or hydroxide by thermal decomposition or by hydrolysis or oxidation of aluminium compounds
  • C01F7/308—Thermal decomposition of nitrates
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
  • C01G25/00—Compounds of zirconium
  • C01G25/02—Oxides
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
  • C01G37/00—Compounds of chromium
  • C01G37/006—Compounds containing, besides chromium, two or more other elements, with the exception of oxygen or hydrogen
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
  • C01G37/00—Compounds of chromium
  • C01G37/14—Chromates; Bichromates
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01G—COMPOUNDS CONTAINING METALS NOT COVERED BY SUBCLASSES C01D OR C01F
  • C01G49/00—Compounds of iron
  • C01G49/0018—Mixed oxides or hydroxides
  • C01G49/0027—Mixed oxides or hydroxides containing one alkali metal
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
  • C01P2004/00—Particle morphology
  • C01P2004/51—Particles with a specific particle size distribution
  • C01P2004/52—Particles with a specific particle size distribution highly monodisperse size distribution
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
  • C01P2004/00—Particle morphology
  • C01P2004/60—Particles characterised by their size
  • C01P2004/62—Submicrometer sized, i.e. from 0.1-1 micrometer
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
  • C01P2004/00—Particle morphology
  • C01P2004/60—Particles characterised by their size
  • C01P2004/64—Nanometer sized, i.e. from 1-100 nanometer
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
  • C01P2006/00—Physical properties of inorganic compounds
  • C01P2006/10—Solid density
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
  • C01P2006/00—Physical properties of inorganic compounds
  • C01P2006/12—Surface area
• • C—CHEMISTRY; METALLURGY
  • C01—INORGANIC CHEMISTRY
  • C01P—INDEXING SCHEME RELATING TO STRUCTURAL AND PHYSICAL ASPECTS OF SOLID INORGANIC COMPOUNDS
  • C01P2006/00—Physical properties of inorganic compounds
  • C01P2006/22—Rheological behaviour as dispersion, e.g. viscosity, sedimentation stability
• • H—ELECTRICITY
  • H01—ELECTRIC ELEMENTS
  • H01M—PROCESSES OR MEANS, e.g. BATTERIES, FOR THE DIRECT CONVERSION OF CHEMICAL ENERGY INTO ELECTRICAL ENERGY
  • H01M2300/00—Electrolytes
  • H01M2300/0017—Non-aqueous electrolytes
  • H01M2300/0048—Molten electrolytes used at high temperature
  • H01M2300/0051—Carbonates

Definitions

• This invention relates to a process for preparing uniform, agglomerate-free, submicron/nanosize ceramic powders for use as starting powders for high technology ceramics.
• this invention relates to a process for preparing uniform, agglomerate-free, submicron/nanosize ceramic powders from a polymeric precursor solution incorporated into a polymeric foam.
• a ceramic powder should consist or dense particles with a narrow size distribution in the submicron range.
• the particles should be discreet, rather than attached together in agglomerated clusters. Agglomerated clusters often produce low-density green ceramics and leave numerous large pores after sintering.
• One known method of preparing powder formulations used in high technology ceramics involves the calcination of a mechanically ground mixture of metal oxides and carbonates in definite proportions.
• the milling and grinding introduces contaminants from abrasive materials which have a detrimental effect on the desirable properties and introduce a variance into each batch of powder prepared.
• the mechanically ground mixture requires prolonged calcination at high temperatures which promotes crystallite coarsening, an undesirable consequence in the fabrication of dense fine grain ceramics.
• Patent 3,330,697 teaches a process for preparing lead and alkaline earth titanates and niobates from resin intermediates made from alpha-hydroxycarboxylic acids, such as citric acid, in which a hydrated oxide or alkoxide and an alpha-hydroxycarboxylate of titanium, niobium, and zirconium is mixed with citric acid in a polyhydroxy alcohol which is liquid below about 100°C, dissolving therein at least one basic one metal compound from the group of oxide, hydroxide, carbonate and alkoxide of lead and the alkaline earth metals, and calcining the composition to remove the organic constituents.
• the resulting product includes agglomerated particles which require grinding after calcination. In addition, particle size is very difficult to control by this method.
• Patent 3,649,354 teaches a method for producing electrically operated devices in which a liquid electrically insulating filler material, such as polyurethane, is applied to a layer of electrically active grains and allowed to contract, thus exposing the peaks of the grains, after which it is allowed to harden.
• U.S. Patent 4,572,843 teaches a method for producing a capacitor in which an insulating composition, such as an organic polymeric compound containing a metal powder or an organometallic compound as a metal source is formed on a dielectric layer formed on an electrode, the insulating composition being heated to form a second conductive electrode.
• U.S. Patent 3,497,455 teaches a method for producing foam metallic oxides in which an aqueous solution of a metal salt (nitrate) is mixed with a frothing agent to form a noncollapsing foam, and subsequently heated up to about 3000°F to form the porous product.
• a metal salt nitrate
• U.S. Patent 4,957,673 teaches a method for producing unitary layered ceramic structures having cosintered layers for use in fuel cells, such as tapes having a center layer of yttria, stabilized zirconia sandwiched between outer layers of strontium doped lanthanum manganite.
• U.S. Patent 2,108,995 teaches an anode of film forming material and a cooperating cathode spaced by a sheet of a flexible nonfibrous albuminous sheet material which has been impregnated and made electrically conductive by the addition of a conductive electrolyte, such as ethylene glycol and citric acid.
• U.S. Patent 2,158,981 teaches an electrolytic condenser having a highly viscous or pasty electrolyte where the electrolyte is, for example, citric acid and ethylene glycol.
• U.S. Patent 3,180,741 teaches a method for producing solid products from liquid polymers with polyvalent metallic salts using a mono- or polycarboxylic acid.
• U.S. Patent 3,386,856 teaches a method for manufacturing a device consisting mainly of oxidic dielectric material in which the device is provided with electrodes and at least one of the surfaces of the device on which the electrodes are provided is superficially oxidized until an insulating junction layer is formed.
• U.S. Patent 3,427,195 teaches a process for producing an electrolytic condenser in which a metal foil is coated with a liquid film of water soluble nitrates or oxalates and finally suspended particles of a water insoluble refractory compound and heated to produce an electrically insulating refractory oxide which, together with a refractory compound, forms the separator coating on the metal foil.
• Patent 4,751,070 which teaches a method for synthesizing submicron particles of ceramic or metallic materials at very low temperatures in which a nitrate source is combined with an inorganic reducing fuel to provide a chemical precursor for the particular ceramic or metallic material, which precursor is exothermically decomposed in a controlled atmosphere at a temperature of about 200°C below the endothermic decomposition temperature of the nitrate source;
• Patent 4,757,037 in which a suspension formed from a mixture of a solution of titania containing elementary crystallites of titanium oxide and a solution of neodymium nitrate or a solution of barium and neodymium nitrates is dried to obtain a dried product and calcined at a temperature of 800° to 1300°C to obtain an ultrafine dielectric powder; U.S.
• Patent 4,800,051 which teaches a method for ceramic fabrication involving hydrolyzing a suitable metal alkoxide to form a slurry, drying the metal oxide powder in the slurry, granulating and calcining the metal oxide powder, ballmilling the calcined metal oxide powder as a slurry to maximize powder dispersion in the solution, compacting the dispersed powder from the ballmilled slurry into a powder compact, drying the powder compact and sintering the powder compact at a suitable relatively low sintering temperature;
• Patent 4,845,056 in which a solution of ceramic oxides or hydrous oxides is continuously pressurized and heated to in excess of the critical temperature and pressure of the solution solvent, transforming the solvent to a gas and subsequently separating it from the fine particulate ceramic oxide powder; and U.S. Patent 4,141,763 in which a stream of an aqueous solution of metal salt and a solution containing a reducing material are injected into a uniformly applied magnetic field from nozzles and immediately mixed as they impinge on one another in the form of sprays to cause a reaction between them.
• none of the prior art teaches a method for preparing uniform, agglomerate free submicron/nanosize ceramic powders by incorporating a precursor solution within a polymeric foam.
• a process for producing ceramic powders in which a polymeric foam comprising metal cations homogeneously incorporated within a foam cell structure of the polymeric foam is calcined in an atmosphere conducive to the removal of the polymeric foam at the lowest temperature and least amount of time required for complete removal of all organics and the formation of the desired crystal phase, preferably, at a calcination temperature of about 400°C to about 1200°C for about 1 ⁇ 2 hour to about 8 hours, producing an oxide powder or a metal powder. If metal powders are desired from the oxide powders produced in accordance with this process, the oxide powders can be reduced to form the desired metal powders.
• metal powders produced in accordance with this process which have a tendency to oxidize upon cooling may be cooled in a reducing atmosphere to prevent oxidation.
• the powders produced in accordance with this process are high purity, uniform, agglomerate-free, nanometer size, multicomponent ceramic/metal powders. Powders produced in accordance with this process range in size from about 5 to about 300 nanometers.
• metal cation salts of the desired ceramic/metal composition are dissolved in a solvent system, such as water, acetone, alcohol or other solvent selected according to its ability to dissolve the metal salts and for its compatibility with the chemicals used to produce the polymeric foam.
• the metal cation solution is then homogeneously mixed with the organic precursors used to produce the polymeric foam.
• the polymeric foam is polyurethane foam and the metal cation solution is homogeneously mixed with the hydroxyl containing component of the components for producing the polyurethane foam, at a ratio determined from the polymerization reaction.
• the resulting chemical solution is then mixed with the other chemical component needed to produce the polyurethane foam at a predetermined ratio.
• the chemical mixture at this stage starts to foam almost immediately at room temperature.
• Hardening occurs during and after the foaming is completed producing metal cations homogeneously incorporated within the vastly expanded, low density polyurethane foam cell structure.
• the hardened foams are then heated above the decomposition temperatures of both the foam and the metal cation salts to form oxide powders of high purity, uniform, nonagglomerated, nanometer size particles.
• Suitable metal cation salts in accordance with this invention are salts which are soluble in a solvent which is compatible with the chemicals used to produce the polymeric foam, such as, chlorides, carbonates, hydroxides, isopropoxides, nitrates, acetates, oxalates, ephoxides and mixtures thereof.
• a solvent which is compatible with the chemicals used to produce the polymeric foam, such as, chlorides, carbonates, hydroxides, isopropoxides, nitrates, acetates, oxalates, ephoxides and mixtures thereof.
• the solvent must not interfere with or destroy the foaming process and/or the polymerization process. It is also preferred that the solvent be completely miscible with one or the other of the chemicals used to produce the polymeric foam.
• a polymeric foam is impregnated with a polymeric precursor solution.
• the impregnated polymeric foam is heated at a temperature between about 80°C to about 150°C to remove the solvent and the solvent-free impregnated polymeric foam is subsequently calcined at a temperature of about 400°C to about 1200°C for about 1 ⁇ 2 to about 8 hours.
• the polymeric precursor solution in accordance with this embodiment of this invention comprises an alpha-hydrocarboxylic acid, a polyhydroxyalcohol and at least one metal cation salt.
• the alpha-hydrocarboxylic acid and the polyhydroxyalcohol form a polymeric resin, the type and amount of which depends on the metal cation salt selected.
• a solvent preferably water, is used to dissolve the metal cation salts and polymeric resin to form a solution.
• a polymeric foam such as a polyurethane foam
• a polymeric foam provides support for the metal cations or polymeric precursor solution so that the metal cations are evenly dispersed within the foam cell structure.
• the physical characteristics of the polymeric foam skeleton such as density, pore size, and pore shape, can be used as a supplemental control for the particle size and morphology of the ceramic powder. Primary control over particle size and morphology is determined by the amount of solvent used to dissolve the cation salts and polymeric resin. Powders produced in accordance with the process of this invention have generally uniform particle sizes between about 5 nanometers up to about 300 nanometers, have no agglomerates and thus require no grinding after calcination, and do not contain impurities introduced by the process.
• a polymeric foam such as polyurethane foam which is known by the inventors to produce favorable results, comprising metal cations homogeneously incorporated within the foam cell structure of the polymeric foam is calcined in an atmosphere conducive to the removal of the polymeric foam, such as air, at a calcination temperature of about 400°C to about 1200°C for about 1 ⁇ 2 hour to about 8 hours.
• a metal cation solution having the desired ceramic/metal composition is mixed with one of the chemical components used for producing the polyurethane foam, preferably the hydroxyl containing component.
• urethane foaming and hardening proceeds in the same way as in the urethane reaction by adding and mixing the hydroxyl containing component with an appropriate amount of the isocyanate containing component. After foaming and hardening, the metal cations are homogeneously incorporated within the vastly expanded, low density polyurethane foam cell structure.
• metal cation salts can be used, such as chlorides, carbonates, hydroxides, isopropoxides, nitrates, acetates, ephoxides, oxalates, and mixtures thereof.
• the type of metal cation salts used are selected on the basis of solubility, preferably having high solubility in a solvent system which is compatible with the compounds used for producing the polyurethane foam. Additional considerations for selecting the cation salts may include low temperature decomposition of the metal salts, environmentally safe composition of the metal salts, and low cost.
• Solvent systems which may be used to dissolve the metal salts comprise water, acetone, and alcohols.
• the preferred solvent system is selected on the basis of its ability to dissolve the desired metal salts and for its compatibility, as previously described, with the compounds used to produce the polyurethane foam.
• the preferred solvent is water which can dissolve a wide variety of metal salts, which is compatible with polyurethane making compounds, which is cheap, and which is environmentally safe.
• Polyurethanes are addition polymers formed by the exothermic reaction of di- or poly-isocyanates with polyols in accordance with the following general reaction:
• water in the system in accordance with this embodiment of the invention is utilized in the polymerization reactions and, thus, may not have to be removed by an extra drying process.
• additives containing only organic substances are preferred to avoid the introduction of impurities.
• polyurethane foam is impregnated with a polymeric precursor solution comprising a polymeric resin and at least one cation salt.
• a polymeric resin known to be effective in accordance with this embodiment of the process of this invention is a mixture of citric acid and ethylene glycol.
• the polymeric resin is mixed with at least one cation salt dissolved in a solvent, preferably water, to form a polymeric precursor solution.
• Impregnation of the polymeric foam can be accomplished in any number of ways, including simply soaking the polymeric foam in the polymeric precursor solution.
• the impregnated polymeric foam is heated at a temperature between about 80°C to about 150°C in a desired atmosphere, preferably air, to drive off the solvent and form dry foam.
• the foam is calcined in a furnace at temperatures between about 400°C to about 1200°C for a period of about 1 ⁇ 2 to about 8 hours, depending on the nature of the ceramic powder and ceramic precursor under preparation and on the particle size desired, in an atmosphere that allows a complete removal of the polymer and decomposition of cation salts.
• a typical heating rate in accordance with one embodiment of the process of this invention is 4°C per minute in a flow of air.
• Ceramic powders obtained after calcination are typically well crystallized, extremely fine and agglomerate-free, requiring no further grinding before being processed and sintered to the desired form.
• This example describes a process for preparing a highly air sinterable La 0.78 Sr 0.22 CrO 3-y (LSC) powder having nonometer size particles which can be used to produce interconnects for a solid oxide fuel cell.
• High purity nitrates, La(NO3)3 ⁇ 6H2O, Sr(NO3)2 and Cr(NO3)3 ⁇ 9H2O were used as the starting materials.
• Appropriate amounts totalling 50 grams of the nitrates were weighed and dissolved in distilled water, approximately 30 grams, in a 600 milliliter glass beaker.
• the metal solution was mixed with 200 milliliters of a mixture of polyols, organic surfactants and catalysts for approximately five minutes.
• the hardened foam was then fired at 750°C, in air, using a heating rate of approximately 5°C per minute and a soaking time of five hours. After the firing, the LSC powder obtained was found to be single phase by x-ray powder diffraction. High resolution SEM showed that the LSC powder had a typical particle size of about 20 nanometers. The powder was essentially nonagglomerated and uniform in size.
• the LSC powder was compacted into a pellet at approximately 130 MPa and sintered in air at 140°C for approximately two hours to produce a sample having 96 percent of theoretical density.
• This is compared to LSC powder prepared using known powder processing methods which produce powders having a particle size of about 1 micron.
• the powders prepared using the known methods require a sintering temperature of about 1700°C under reducing atmosphere conditions to obtain a similar density.
• This example demonstrates a process for preparing nanometer size 8 mole percent Y2O3 stabilized ZrO2 (ysz), which is used in structural ceramics, sensors, and electrolytes in solid oxide fuel cells.
• the starting materials used were ZrO(NO3)3 ⁇ xH2O and Y(NO3)3 ⁇ xH2O.
• About 50 grams of the nitrates, in a stoichiometric ratio required to obtain Zr 0.84 Y 0.16 O 1.92 was dissolved in approximately 40 grams of distilled water.
• the nitrate solution was mixed in a 600 milliliter glass beaker with a mixture of polyols, organic surfactants and catalysts for approximately five minutes. Polymeric isocyanates were added to the mixture and mixed for approximately one minute and the resulting chemical mixture was transferred to two 2L size porcelain dishes where foaming rapidly occurred. The foam hardened after about thirty minutes and was fired at 750°C, in air, for five hours.
• the powder thus obtained exhibited a single cubic phase of ysz as shown by x-ray powder diffraction.
• BET study showed that the ysz powder had a surface area of 96 meters squared per gram.
• SEM studies showed that the powder had a particle size of about 20 nanometers.
• the powder was subsequently die pressed at about 130 MPa and sintered at 1250°C for one minute. A density of about 90 percent of the theoretical value was obtained. When sintered at 1350°C, ceramics close to the theoretical density, approximately 96 percent of theoretical density, were obtained.
• the solvent system used contained ethanol and acetone in a one to one ratio. All preparative procedures were similar to the procedure described in Example II above. A BET surface area of 104 square meters per gram was measured and SEM micrographs showed particle sizes of about 20 nanometers.
• This example demonstrates a process for preparing nanometer size Al2O3 which is widely used as a structural ceramics.
• the starting material used was Al(NO3)3 ⁇ H2O.
• About 50 grams of the nitrate was dissolved in approximately 40 grams of distilled water.
• the nitrate solution was mixed in a 600 milliliter glass beaker with a mixture (about 150 grams) of polyols, organic surfactants and catalysts for approximately five minutes.
• Polymeric isocyanates (about 150 grams) were added to the mixture and mixed for approximately one minute and the resulting chemical mixture was transferred to two 2L size porcelain dishes where foaming rapidly occurred.
• the foam hardened after about 30 minutes and was fired at 750° C, in air, for 3 hours.
• the powder thus obtained has a BET surface area of about 118 m2/grams. This corresponds to an average particle diameter of about 13 nm.
• This example demonstrates a process for preparing uniform, submicron LiFeO2 powder as electrode materials for use in a molten carbonate fuel cell.
• the starting materials used were LiNO3 and Fe(NO3)3 ⁇ 9H2O.
• the nitrate solution was mixed in a 600 milliliter glass beaker with a mixture (about 150 grams) of polyols, organic surfactants and catalysts for approximately five minutes.
• Polymeric isocyanates (about 150 grams) were added to the mixture and mixed for approximately one minute and the resulting chemical mixture was transferred to two 2L size porcelain dishes where foaming rapidly occurred.
• the foam hardened after about 30 minutes and was fired at 750° C, in air, for 3 hours.
• the powder thus obtained has a BET surface area of about 3.8 m2/grams. This corresponds to an average particle diameter of about 0.36 micron. An average particle size of about 0.3 to 0.4 micron was observed using SEM.
• This example describes a process for preparing a submicron, nonagglomerated and highly air sinterable La 0.78 Sr 0.22 CrO 3-y powder which can be used to produce interconnects for solid oxide fuel cells.
• An appropriate amount of high purity nitrates La(NO3)3 ⁇ H2O, Sr(NO3)2 and Cr(NO3)3 ⁇ 9H2O were weighed and dissolved in distilled water. The nitrates to water ratio was 1:1 by weight.
• Citric acid was also dissolved in a small amount of water, mixed with ethylene glycol and finally added to the nitrate solution to obtain a polymeric precursor solution of La(Sr)CrO3.
• Sample pellets of the resulting powder 12.7 millimeters in diameter and 2 millimeters thick, were obtained by die pressing at about 130 MPa. A green density of about 50 percent of the theoretical was obtained. Sintering was carried out at various temperatures from 1400° to 1600°C in air for six hours with a heating rate of 20°C per minute. The final densities of the samples were measured using the water immersion method with the following results: As shown, the lanthanum strontium chromate powder prepared using this embodiment of the process of this invention can be sintered to a density of about 92 percent at 1400°C in air. In contrast thereto, a lanthanum strontium chromate powder prepared from the same polymeric precursor solution without a foam skeleton support during drying and calcination can only be sintered to less than 80 percent density at 1600°C.

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